Consider the following equilibrium: 2NO₂ (g) N₂O4 (g) - AG=- = -5.4 kJ Now suppose a reaction vessel is filled with 0.974 atm of nitrogen dioxide (NO₂) at 1003. °C. Answer the following questions about this system: Under these conditions, will the pressure of NO₂ tend to rise or fall? Is it possible to reverse this tendency by adding N₂O4? In other words, if you said the pressure of NO₂ will tend to rise, can that be changed to a tendency to fall by adding N₂O4? Similarly, if you said the pressure of NO₂ will tend to fall, can that be changed to a tendency to rise by adding N₂O4? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂O4 needed to reverse it. Round your answer to 2 significant digits. O rise fall yes no atm x10 X
Consider the following equilibrium: 2NO₂ (g) N₂O4 (g) - AG=- = -5.4 kJ Now suppose a reaction vessel is filled with 0.974 atm of nitrogen dioxide (NO₂) at 1003. °C. Answer the following questions about this system: Under these conditions, will the pressure of NO₂ tend to rise or fall? Is it possible to reverse this tendency by adding N₂O4? In other words, if you said the pressure of NO₂ will tend to rise, can that be changed to a tendency to fall by adding N₂O4? Similarly, if you said the pressure of NO₂ will tend to fall, can that be changed to a tendency to rise by adding N₂O4? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂O4 needed to reverse it. Round your answer to 2 significant digits. O rise fall yes no atm x10 X
Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter17: Equilibrium
Section: Chapter Questions
Problem 126CP: . Consider the following exothermic reaction at equilibrium: N2(g)+3H2(g)2NH3(g)Predict how the...
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